Theoretical inorganic chemistry pH of aqueous solutions of hypophosphites

@damiryagudin Internet resources, tutorials (Tretyakov)

@argentum mean, if we compare the strength of acids, it is better to give their dissociation constants (acidity constants), and not the dissociation constant index. Still, for comparison, I would use the dissociation constant itself. There the difference will be more noticeable. Although of course this indicator is used for convenience, but still it is a decimal logarithm, and not the value of the dissociation constant itself.

Are you sure it's H₃PO₂ a weak acid?

@damiryagudin  K₁ H₃PO₃ = 5,1⋅10⁻²
 K H₃PO₂ = 8,9․10^-2

@damiryagudin it's all relative, the question is that it is comparable in strength to phosphorous acid

@argentum Judging by the dissociation constant of H₃PO_2, acid is definitely not weak. If we calculate the hydrolysis constant, it is much less than the acid dissociation. Therefore, the hydrolysis of hypophosphites does not occur.

H₃PO₃ acid dissociates stepwise. Comparing the dissociation constant of H₃PO₃  at the first stage with H₃PO₂ , which, as you say, are close, it can be concluded that acid salts of H₃PO₃(hydrophosphites MeH(HPO₃)) will not undergo hydrolysis. But the average salts of H₃PO₃ (phosphites Me₂(HPO₃)) in an aqueous solution will already be hydrolyzed by anion to form an alkaline medium (K2 = 2∙10-7).

And as a fact, I would not rely on one source of literature at all. It is clear that it is conditional, but still, I would look for information about the strength of acids.

@damiryagudin Thank you for your well-reasoned and detailed answer!